Question Bank › Physical Chemistry › Electrochemistry › ABC26PH0390In the mixture obtained by mixing 25.0 mL 1.2 × 10⁻³ M MnCl₂ and 35.0 mL of 6.0 × 10⁻⁴ M KCl solution, the… · ABC26PH0390 Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Electrochemistry – General · Exam: GATE 2005-2021 · Marks: 2 · Difficulty: Medium
In the mixture obtained by mixing 25.0 mL $1.2 \times 10^{-3}$ M $\mathrm{MnCl_2}$ and 35.0 mL of $6.0 \times 10^{-4}$ M KCl solution, the concentrations (M) of $\mathrm{Mn^{2+}}$, $\mathrm{K^+}$ and $\mathrm{Cl^-}$ ions respectively are
(a) $6.0\times10^{-4}, 3.0\times10^{-4}, 1.5\times10^{-3}$
(b) $6.0\times10^{-4}, 3.0\times10^{-4}, 9.0\times10^{-4}$
(c) $5.0\times10^{-4}, 3.5\times10^{-4}, 1.35\times10^{-3}$
(d) $5.0\times10^{-4}, 3.5\times10^{-4}, 8.5\times10^{-4}$
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